General Chemistry Exam 1 Review Guide: Key Concepts and Study Notes

Study Guide - Smart Notes

Tailored notes based on your materials, expanded with key definitions, examples, and context.

Green chemistry focuses on designing products and processes that minimize environmental impact and reduce the use of hazardous substances.

Green Chemistry Principles: Reduce waste, use renewable resources, and design safer chemicals.
Sustainable Chemistry: Integrates environmental, economic, and social considerations into chemical research and production.
Scientific Method: A systematic approach to research involving observation, hypothesis, experimentation, and conclusion.
Scientific Theory vs. Law: A theory explains why phenomena occur; a law describes consistent relationships under certain conditions.

Example: The development of biodegradable plastics using renewable resources is an application of green chemistry.

Atoms are composed of protons, neutrons, and electrons. The arrangement and number of these particles determine the properties of elements.

Example: Carbon-12 has 6 protons, 6 neutrons, and 6 electrons.

Isotopes: Atoms of the same element with different numbers of neutrons.
Ions: Atoms or molecules that have gained or lost electrons, resulting in a net charge.

Example: Na+ is a sodium ion formed by losing one electron.

Chemical bonds are forces that hold atoms together in compounds.

Example: Sodium chloride (NaCl) is formed by the transfer of an electron from sodium to chlorine.

The periodic table organizes elements by increasing atomic number and similar chemical properties.

Groups: Vertical columns with similar properties.
Periods: Horizontal rows indicating energy levels.
Trends: Atomic radius, ionization energy, and electronegativity change predictably across periods and groups.

Example: Alkali metals (Group 1) are highly reactive and have low ionization energies.

The mole is a fundamental unit for counting atoms, molecules, or ions in chemistry.

Avogadro's Number: particles per mole.
Molar Mass: The mass of one mole of a substance, expressed in grams per mole (g/mol).

Example: One mole of water (H2O) contains molecules and has a mass of 18.02 g.

Stoichiometry involves calculations based on balanced chemical equations to determine the quantities of reactants and products.

Balanced Equation: Ensures the same number of each atom on both sides of the reaction.
Limiting Reactant: The reactant that is completely consumed first, limiting the amount of product formed.
Theoretical Yield: Maximum amount of product that can be formed from given reactants.
Percent Yield:

The physical properties of matter depend on the arrangement and motion of particles.

Solids: Particles are closely packed in a fixed arrangement; definite shape and volume.
Liquids: Particles are close but can move past each other; definite volume, no definite shape.
Gases: Particles are far apart and move freely; no definite shape or volume.

Dipole-Dipole Forces: Attractions between polar molecules.
Dispersion (London) Forces: Weak attractions due to temporary dipoles in all molecules.
Hydrogen Bonds: Strong dipole-dipole attractions involving H bonded to N, O, or F.

Example: Water's high boiling point is due to hydrogen bonding.

The ideal gas law relates the pressure, volume, temperature, and amount of a gas.

Equation:
P: Pressure (atm), V: Volume (L), n: Moles, R: Gas constant (0.0821 L·atm/mol·K), T: Temperature (K)
Given any three variables, the fourth can be calculated.

Example: Calculate the volume occupied by 2 moles of an ideal gas at 1 atm and 273 K.

Type of Force	Occurs Between	Relative Strength	Example
Dipole-Dipole	Polar molecules	Moderate	HCl
Dispersion (London)	All molecules	Weakest	O2, N2
Hydrogen Bond	H with N, O, or F	Strongest	H2O, NH3

These notes are structured to cover the main learning outcomes for a General Chemistry exam, including atomic structure, chemical bonding, periodic trends, chemical calculations, states of matter, intermolecular forces, and gas laws.
Students should be familiar with using a calculator for stoichiometric and gas law calculations.